Given below are two statements: Statement-I: The correct order in terms of atomic/ionic radii is textAl > textMg > textMg^2+ > textAl^3+$\text{Al} > \text{Mg} > \text{Mg}^{2+} > \text{Al}^{3+}$. Statement-II: The correct order in terms of the magnitude of electron gain enthalpy is textCl > textBr > textS > textO$\text{Cl} > \text{Br} > \text{S} > \text{O}$. In the light of the above statements, choose the correct answer from the options given below:

### Core Logic - Statement I: Correct order of size is textMg > textAl > textMg^2+ > textAl^3+$\text{Mg} > \text{Al} > \text{Mg}^{2+} > \text{Al}^{3+}$ because atomic radius of magnesium is greater than aluminium in period 3. Thus Statement-I is false. - Statement-II: Chlorine has the highest electron gain enthalpy in the periodic table, and halogens exceed chalcogens. The order textCl > textBr > textS > textO$\text{Cl} > \text{Br} > \text{S} > \text{O}$ is true. ### Step 1: Final Conclusion Statement I is false but Statement II is true, corresponding to option (2). ### Pattern Recognition Sees: Periodic trends for atomic radii and electron affinity. Trap: Assuming Al is larger than Mg due to higher atomic number. ### Chapter Mix Class 11 Chemistry: Classification of Elements and Periodicity in Properties